Effective Biosorption of Nickel(II) From Aqueous Solutions Using Trichoderma Viride

Hindawi Publishing CorporationJournal of ChemistryVolume 2013 Article ID 716098 7 pageshttpdxdoiorg1011552013716098

Research ArticleEffective Biosorption of Nickel(II) from Aqueous Solutions UsingTrichoderma viride

P Sujatha1 V Kalarani1 and B Naresh Kumar2

1 Department of Biotechnology Sri Padmavati Mahila Visvavidyalayam (Womenrsquos University) Andhara PradeshTirupati 517502 India

2 Food and Water Division Vimta Life Sciences Hyderabad 500078 India

Correspondence should be addressed to V Kalarani kaladandalagmailcom

Received 19 February 2012 Revised 27 June 2012 Accepted 7 August 2012

Academic Editor Veysel T Yilmaz

Copyright copy 2013 P Sujatha et alis is an open access article distributed under theCreativeCommonsAttributionLicense whichpermits unrestricted use distribution and reproduction in any medium provided the original work is properly cited

e primary objective of the present study is to evaluate the optimization conditions such as kinetic and equilibrium isothermmodels involved in the removal of Ni(II) from the aqueous solutions by Trichoderma viride e biosorbent was characterized byFTIR and SEM e optimum biosorption conditions were determined as a function of pH biomass dosage contact time initialmetal ion concentration and temperature e maximum Ni(II) biosorption was obtained at pH 45 e equilibrium data werebetter t by the Langmuir isothermmodel than by the Freundlich isotherme kinetic studies indicate that the biosorption processof the metal ion Ni(II) has followed well the pseudo-second-order model e sum of the square errors (SSE) and chi-square (1205941205942)tests were also carried out to nd the best t kinetic model and adsorption isotherm e maximum biosorption capacity (119902119902119898119898) ofT viride biomass was found to be 476mgg for Ni(II) ion erefore it can be concluded that T viride biomass was effective andlow-cost potential adsorbent to remove the toxic metal Ni(II) from aqueous solutionse recovery process of Ni(II) from T viridebiomass was found to be higher than 98 by using 025M HNO3 Besides the application of removal of toxic metal Ni(II) fromaqueous solutions the biosorbent T viride can be reused for ve consecutive sorption-desorption cycles was determined

1 Introduction

Metal pollution has been a great concern for the past fewdecades It is believed that the wide use of man-made chemi-cals anthropogenic lifestyle and rapid industrialization is themajor source of metal toxicity [1] Nickel is well known as aheavy metal pollutant present in effluents of electroplatingindustries smelting and alloy manufacturing mining andrening industries [2] According to WHO the permissi-ble limit of Ni(II) in drinking water is 05mgL [3] enon-biodegradable and bioaccumulating properties of heavymetals may pose serious threats to living organisms [4] Ithas been reported that both occupational and environmentalexposure to trace metals affects almost all compartmentsof animal systems including human health [1] In humansand animals nickel is an essential micronutrient [5] becauseof its importance in the metabolic pathways Nickel is oneof the cofactors for urease enzyme in plants [6] oughit is an essential micronutrient andor cofactor nickel is

one of the heavy metal toxicants at higher concentrationand is a well-known human carcinogen [7] Nickel hasbeen implicated as an embryotoxin and teratogen [8] ehigher concentration of Nickel causes dermatitis nauseavomiting behavioral and respiratory problems in additionto cyanosis gastrointestinal distress and weakness [9] Allthese biological disorder consequences alarm the need ofnickel removal from the environment and to bring upits levels below the threshold limits from its sources eclassical physicochemical methods are commonly used forthe removal of nickel from the industrial effluents namelyevaporative recovery ltration ion exchange andmembranetechnologies ough they are promising to some extent butthese processes have high reagent or energy requirementsand generate toxic sludge that requires careful disposal [10]Furthermore insufficient removal of traces of heavy metalions varying performances and also high operating costs haslimited the use of conventional physicochemical methodsus there is a need for alternativemethods for better efficacy

2 Journal of Chemistry

with low cost and complete removal of toxic metals from thewater bodies

In recent years the exploitation of eco-friendly biosorp-tion technology using inactive and dead biomasses to detox-ify metal-contaminated effluents in the aquatic environmentis gaining importance day by day [11 12] Moreover thebiosorbents have high specic metal binding ability incomplex media in contrast to carbonaceous sorbents whichtend to adsorb metal ions in a nonspecic manner eseadvantages make biosorbents an economical alternative tocommercial activated carbons in the removal of heavy metal-polluted water bodies [13]

e application of fungal organisms in the eld ofbiosorption technology has become a part of active researchby the environmental scientists Fungal organisms likeAspergillus niger [14] Streptomyces noursei [15] Pseu-domonas aeruginosa [16] and Rhizopus arrhizus [17] havebeen reported for removal of heavy metals such as PbCd and in particular Ni(II) Among the fungal organismsthe T viride in biosorption process is little exploited [18]e present study in our laboratory is mainly aimed atknowing the application of T viride for sequestration ofNi(II) from contaminated water systems involving kineticand equilibrium e selection of this biosorbent T virideis based on (1) inexpensive (2) easily available (3) no toxiceffects of its own and (4) some information suggests thatmetal-bioaccumulation properties of T viride [19] Hencestudies on the kinetic and equilibrium isotherm modelshave been studied in order to systematically investigatethe application of biomass T viride as biosorbent for theremoval of nickel ions from waterindustrial waste watere optimum conditions for biosorption such as pH initialmetal ion concentration biomass dosage contact time andequilibrium isotherm models in relation to the biosorptionof Ni(II) onto T viride have been investigated In addition tothis the Ni(II) ion desorption studies have been performedover ve sorption-desorption cycles to evaluate the sorbentT viride for reusage

2 Experimental

21 Collection and Preparation of Biomass (Adsorbent) efungal biomass was collected from Microbial Type CultureCollection (MTCC) Chandigarh India e biomass wasprepared in the sabouraud broth (peptone 100 dextrose400 streptomycin 003 and agar 200 gL) by inoculating the01mL spore suspension100mLofwater in the 250mLasksand incubated at room temperature for 5ndash7 days Sampleswere washed several times using deionized water to removeadhesive materials such as extraneous salts and then dried inoven at 60∘C for 48 h and powdered to uniform size using amortar

22 Reagents and Equipments A ame atomic absorptionspectrophotometer (Shimadzu AA-6300 Japan) with nickelhallow cathode lamp was used for determination of Ni(II)before and aer biosorption Absorbance was measured atwavelength of 232 nm and spectral bandwidth was 02 nm

Tra

nsm

itta

nce

(

)

4000 3000 2000 1500 1000 500

33

54

29

24

16

53

14

49 12

44

10

28

63

3

Wavenumber (cmminus1)

(a) Unloaded

Tra

nsm

itta

nce

(

)

3332

2925

16

42

14

36 1

20

2 57

6

1079

4000 3000 2000 1500 1000 500


(b) Total nickel loaded

F 1 FTIR spectra of T viride biomass before adsorption (a)and aer adsorption of Nickel (b)

Fourier Transform Infrared (FT-IR) spectrometer (ermo-Nicolet FT-IR Nicolet IR-200 USA) was used for IR spectralstudies of dried biomass and Ni(II)-sorbed biomass in therange of 4000ndash400 cmminus1 and Scanning Electron Microscopy(SEM Model Evo15 Carl Zeiss England) has been used tostudy the surface morphology of the biosorbent

3 Results and Discussion

31 Characterization of Biomass e FTIR spectra of freebiomass and nickel sorbed biomass samples were showedin Figure 1 e spectra of free biomass (Figure 1(a)) hasshown a broad and strong peak at 3354 cmminus1 which maybe due to the overlapping of OndashH and NndashH stretchingvibrations e peak at 2924 cmminus1 can be assigned to thendashCH groups of an unloaded biomass sample e peaks at1642 and 1653 cmminus1 may be attributed to asymmetric andsymmetric stretching vibration of C=O groups respectivelye spectrum of nickel sorbed biomass (Figure 1(b)) hasrevealed that the bands that have been observed at 3332 14361202 and 1079 cmminus1 for free biomass are shied to 33541449 1244 and 1028 cmminus1 e signicant changes in thewave numbers of these specic peaks have suggested thatamine hydroxyl C=O and alcoholic CndashO groups of biomasscould be involved in the biosorption of nickel ion onto Tviride

Figure 2 shows the morphology of T viride before andaer biosorption of Ni(II) Before Ni(II) biosorption on Tviride shows adhesive and small particles (Figure 2(a)) It hasbeen shown that the morphology changed to a corn ake-like structure aer Ni(II) biosorption onto T viride biomass

Journal of Chemistry 3

(a)

(b)

F 2 SEM micrographs of T viride biomass surface (a) beforeadsorption of Ni(II) ions and (b) aer adsorption of Ni(II) ions

(Figure 2(b)) It can be seen that the surface modicationsoccurred by reducing the irregularity aer binding of Ni(II)ions onto the surface T viride biomass

32 Effect of PH Biosorption of Ni(II) onto biomass of Tviride as a function of initial pH has been shown in Figure3 It has been observed that the biosorption capacity isincreased from pH 20 to 45 Beyond pH 45 the biosorptionhas gradually decreased At lower pH the cell wall of Tviride becomes positively charged due to the increase inhydrogen ion concentration which is responsible for reduc-tion in biosorption of Ni(II) ions on adsorption sites Incontrast at higher pH (gt45) the cell wall surface becomesmore negatively charged when compared to surface negativecharges at lower pH At pH greater than 45 nickel ions startbinding with OHminus forming the insoluble nickel hydroxidesthat resulted in the reduction of biosorption

33 Effect of Biosorbent Dose on Biosorption e biosorbentdosage is an important parameter which determines the

100

90

80

70

60

50

40

Ad

sorp

tio

n c

apac

ity

(mg

gminus

1)

0 1 2 3 4 5 6 7

(pH)

F 3 Effect of pH on the biosorption of Ni(II) onto T viridebiomass

Amount of adsorbent (g)

50

60

70

80

90

100

110

0 01 02 03 04 05 06 07 08

Rem

ova

l (

)

F 4 Effect of biosorbent dosage level on the biosorption ofNi(II) T viride biomass

capacity of a biosorbent for a given initial concentratione biosorption of Ni(II) ion as a function of the biosor-bent dosage of 01 g to 07 g has been investigated and theresults are shown in Figure 4 e percentage of biosorptionhas increased with the increase of biosorbent dose up to05 g01 L At the initial concentration of 100mgL of Ni(II)the maximum percentage removal was 923 and remainedconstant at gt05 g01 L erefore the optimum biosorbentdosage was taken as 05 g for further experiments to deter-mine the effect of contact time biosorption kinetics andbiosorption isotherm models

34 Effect of Contact Time e biosorption capacity of Tviride towards Ni(II) was investigated at different initialconcentrations and xed amount of fungi at different timeintervals e efficacy of biosorption increases with agitationtime and reached equilibrium about 180min for all the exper-imental concentrations performed e rate of the uptake ofmetal ions was rapid in the early stages as expected then theequilibrium was attained due to continuous formation of the


T 1 Kinetic parameters for biosorption of Ni(II) by T viride biomass

Metal ion Lagergren rst order Pseudo second order Weber and Morris1198701198701 (minminus1) 1198771198772 SSE 1198701198702 (g(mgmin)) 1198771198772 SSE 119870119870id (mggminminus05) 1198771198772 SSE00165 09982 0995 00004 0999 0011 2328 09498 0922

Ni(II) 00158 09856 0998 00004 0997 0003 2934 09877 094300127 09921 0999 00004 0997 0004 3809 09869 095100134 09968 0999 00004 0999 0003 4559 09713 0934

biosorption layer until saturation e data obtained fromthe experiment has been further used to evaluate the kineticparameters of the biosorption process

35 Biosorption Kinetics e mechanism of biosorptiondepends on the physical and chemical characteristics of theadsorbents as well as on the mass transfer process [20]e results of rate kinetics of Ni(II) biosorption onto Tviride biomass are analyzed using pseudo-rst-order pseudo-second-order and intraparticle diffusion models e con-formity between experimental data and the model predictedvalues was expressed by correlation coefficients (R2)

e linear pseudo-rst-order model [21] can be repre-sented by the following equation

log 10076491007649119902119902119890119890 minus 11990211990211990511990510076651007665 = log 119902119902119890119890 minus11989611989611199051199052303 (1)

where 119902119902119890119890 (mgg) and 119902119902119905119905 (mgg) are the amounts of adsorbedmetal on the sorbent at the equilibrium time and at any timet respectively and 1198961198961 is the rate constant of pseudo-rst-order adsorption process (minminus1)e experimental data wastted to (1) and various parameters obtained for biosorptionof Ni(II) onto T viride with different initial concentrationstogether with correlation coefficients are given in Table 1ecorrelation coefficients for the pseudo-rst-order equationobtained at all the studied concentrations were low issuggests that this biosorption systemdoes not follow the rst-order reaction

e kinetics of biosorption process may also be describedby pseudo-second-order rate equation [22] e lineralizedform of equation was given as follows

119905119905119902119902119905119905=111989611989621199021199022119890119890+1119902119902119890119890119905119905 (2)

where 1198961198962 (g(mg min)) is the equilibrium rate constant ofpseudo-second-order biosorptione pseudo-second-orderequation parameters obtained for biosorption of Ni(II) ontoT viride with different initial concentrations together withcorrelation coefficients are given in Table 1

e biosorption results were analyzed using intraparticlediffusion model [23] is is represented as

119902119902119905119905 = 119896119896id11990511990505 + 119888119888 (3)

where 119902119902119905119905 (mgL) is the amount adsorbed at time t (min)and 119896119896id (mgg minminus05) is the rate constant of intraparticlediffusionC is the value of intercept which gives an idea aboutthe boundary layer thickness that is the larger intercept

200

180

160

140

120

100

80

60

40

20

0qt

(mg

gminus

1)

0 2 4 6 8 10 12 14 16

t12

50

100

150

200

F 5 Weber and Morris plots for the biosorption of Ni(II) Tviride biomass

the greater is the boundary effect e Weber Morris plotfor biosorption of Ni(II) is given in Figure 5 Based on theresults it can be concluded that both lm diffusion andintraparticle diffusion are simultaneously operating duringthe biosorption of Ni(II) onto T viride biomass

36 Fitness of the Biosorption Kinetic Models e values ofrate constants and correlation coefficients for each modelwere shown in Table 1 e best t among the kinetic modelsis assessed by the squared sum of error (SSE) values It isassumed that the model which gives the lower SSE values isthe best model for metal ion sorption on T viride e SSEvalues are calculated by the following equation

SSE = 100557610055761007657100765710076501007650119902119902119905119905119890119890 minus 11990211990211990511990511990511990510076661007666

2

119902119902210076731007673 (4)

where 119902119902119905119905119890119890 and 119902119902119905119905119905119905 are the experimental biosorption capac-ities of metal ions (mgg) at time t and the correspondingvalues that are obtained from the kinetic models SSE valuesfor all the kinetic models are calculated and summarizedin Table 1 e lower SSE values of pseudo-second-ordermodel indicate that the biosorption of Ni(II) on the T viridebiosorbent follows the pseudo-second-order kinetic model

37 Biosorption Isotherms Models e equilibrium adsorp-tion isotherm is of importance in the design of adsorption


systems [24]e adsorption isotherms for Ni(II) adsorptiononto T viride biomass at the temperature of 20 30 and 40∘Care shown in Figures 6(a) and 6(b) e Langmuir treatmentis based on the assumption that the maximum adsorptioncorresponds to a saturated monolayer of solute moleculeson the adsorbent surface that the energy of adsorption isconstant and there is no transmigration of adsorbate in theplane of the surface [25] It is represented by

119902119902119890119890 =1199021199021198981198981198701198701198711198711198621198621198901198901 + 119870119870119871119871119862119862119890119890

(5)

where 119902119902119890119890 is the equilibrium metal ion concentration on thesorbent (mgg)119862119862119890119890 is the equilibriummetal ion concentrationin the solution (mgL) 119902119902119898119898 is the monolayer sorption capacityof the sorbent (mgg) and 119870119870119871119871 is the Langmuir sorptionconstant (Lmg) related to the free energy of sorption Figure6(a) shows the Langmuir plots at different temperatures andthe constants 119902119902119898119898 and 119870119870119871119871 are tabulated in Table 2 On theother hand Table 3 presents the comparison of biosorptioncapacity (mgg) ofT viride for Ni(II) ions with that of variousbiosorbents reported in the literature [26ndash28]

e general form of Freundlich is given as follows

119902119902119890119890 = 1198961198961198911198911198621198621119899119899119890119890 (6)

where 119870119870119891119891 is a constant related to the biosorption capacityand 1n is an empirical parameter related to the biosorptionintensity which varies with the heterogeneity of the materialFigure 6(b) shows the Freundlich plots at different tempera-tures and the constant 119870119870119891119891 and 1n are tabulated in Table 2e best t biosorption isotherm model is conrmed by thecorrelation coefficients (1198771198772) and the chi-square (1205941205942) testseequation for evaluating the best t model is to be written as

1205941205942 = 100557610055761007657100765710076501007650119902119902119890119890 minus 11990211990211989011989011989811989810076661007666

2

11990211990211989011989011989811989810076731007673 (7)

where q 119890119890 is the experimental data of the equilibriumcapacity (mgg) and q 119890119890119898119898 is equilibrium capacity obtained bycalculating from themodel (mgg) 1205941205942 will be a small numberif the data from the model are similar to the experimentaldata while 1205941205942 will be a bigger number if they differ usit is also necessary to analyse the data set using the nonlinear1205941205942 test to conrm the best-t isotherm for the biosorptionprocess and the1205941205942 values are given in Table 2e1205941205942 values ofboth isotherms are comparable and hence the adsorption ofmetal ions follows both Freundlich and Langmuir isothermsand better t to Langmuir as its 1205941205942 value is less than that ofthe Freundlich model

38 Desorption Experiment In addition to biosorption stud-ies desorption processes have equal importance due to thereusage of biomass material Desorption mainly dependsupon (a) type of eluents and (b) biomass material used Inthe present study HNO3 solution was used as the eluentto remove Ni(II) from T viride Different concentrations

008

007

006

005

004

003

002

001

0

1q

e

1Ce

0 005 01 015 02 025

(a)

2

18

16

14

12

1

08

06

04

02

0

logqe

logCe

0 02 04 0806 1 12 14 16

(b)

F 6 (a) Langmuir isotherm plots for the biosorption of Ni(II)T viride biomass at different temperatures (b) Freundlich isothermplots for the biosorption of Ni(II) T viride biomass at differenttemperatures

(001ndash04M) were used to desorb the Ni(II)-T viride com-plexe results of the present study indicate that the additionof acid at lower concentration 001M HNO3 desorbs thenickel from the complex and gt55 adsorption was observedat 005MHNO3 emaximum desorption (gt98) of nickelfrom the complex occurs at gt025M HNO3

39 Recovery of Ni(II) by Adsorption-Desorption Cycle Inorder to evaluate the reutilization of the T viride thebiosorption-desorption cycles are repeated ve times bytreating the used biosorbent with 025M HNO3 e des-orption efficiency of 9977 of Ni(II) was obtained by using025M HNO3 in the rst cycle and is therefore suitable forregeneration of biosorbent ere was a gradual decrease of


T 2 Langmuir and Freundlich isotherm parameters for the biosorption of Ni(II) on Tviride biomass at different temperatures

Metal ion Temperatures (119870119870) Langmuir Freundlich119902119902max (mgg) 119870119870119871119871 (Lmg) 1198771198772 1205941205942 119870119870119891119891 (mgg) 119899119899 1198771198772 1205941205942

293 263 257 0999 1125 4538 1174 0993 512Ni(II) 303 370 315 0999 1728 3566 11047 0999 621

313 476 368 0999 2167 2875 1076 0999 699

T 3 A comparison of biosorption capacity (mgg) of differentbiomasses for Ni(II) removal

Biomass 119902119902119898119898 (mgg) ReferencesRhizopus nigricans 5 [26]Streptomyces noursei 08 [26]Waste pomace of olive factory 1480 [27]PAC (Powdered activated carbon) 3108 [28]T viride 476 (Present study)

Ni(II) biosorption on T viride with an increase the numberof desorption cycles Aer a sequence of ve cycles it wasobserved that the Ni(II) uptake capacity of the T viridehas been reduced from 9815 to 9513 e desorptionefficiency more than 98 recovery of Ni(II) was observed ineach cycle of all the ve consecutive desorption cycles eresults indicate that the T viride can be used repeatedly inthe adsorption-desorption cycles

4 Conclusion

is study is focused on the biosorption of Ni(II) ion ontoT viride biomass from aqueous solution e operatingparameters pH of solution biomass dosage contact timeinitial metal ion concentration and temperature are effectiveon the biosorption efficiency of Ni(II) e biosorptioncapacity of T viride biomass has been found to be 476mggfor Ni(II) Langmuir model has tted the equilibrium databetter than the Freundlich isotherm e kinetic data hasillustrated that pseudo-second-order model is more suitablethan a pseudo-rst-order model based on the lower SSE andcorrelation coefficients that are greater than 099 T viridecan be used for 5 cycles by regenerating with 025M HNO3Further it can be evaluated as an alternative biosorbentto treat wastewater containing Ni(II) ion over the classicalphysicochemical methods Hence T viride can be used asan effective low-cost biosorbent for potential removal ofheavy toxic metal Ni(II) from aqueous mediae signicantadvantage of T viride is reusage of it when compared to othermethods using different types of fungi for removal of Ni(II)from water media

References

[1] J Wang and C Chen ldquoBiosorbents for heavy metals removaland their futurerdquo Biotechnology Advances vol 27 no 2 pp195ndash226 2009

[2] E Denkhaus and K Salnikow ldquoNickel essentiality toxicity andcarcinogenicityrdquo Critical Reviews in OncologyHematology vol42 no 1 pp 35ndash56 2002

[3] World Health Organization Guidelines for Drinking-WaterQuality Incorporating First addendum to ird Edition vol 1World Health Organization Geneva Switzerland 3rd edition2006

[4] Y Liu and H Xu ldquoEquilibrium thermodynamics and mech-anisms of Ni2+ biosorption by aerobic granulesrdquo BiochemicalEngineering Journal vol 35 no 2 pp 174ndash182 2007

[5] E O Uthus and C D Seaborn ldquoDeliberations and evaluationsof the approaches endpoints and paradigms for dietary recom-mendations of the other trace elementsrdquo Journal of Nutritionvol 126 no 9 supplement pp 2452Sndash2459S 1996

[6] R KWatt and PW Ludden ldquoNickel-binding proteinsrdquoCellularand Molecular Life Sciences vol 56 no 7-8 pp 604ndash625 1999

[7] M G Maleva G F Nekrasova P Malec M N V Prasad andK Strzałka ldquoEcophysiological tolerance of Elodea canadensis tonickel exposurerdquoChemosphere vol 77 no 3 pp 392ndash398 2009

[8] C-Y Chen and T-H Lin ldquoNickel toxicity to human termplacenta in vitro study on lipid peroxidationrdquo Journal ofToxicology and Environmental Health A vol 54 no 1 pp37ndash47 1998

[9] N Akhtar J Iqbal and M Iqbal ldquoRemoval and recovery ofnickel(II) from aqueous solution by loofa sponge-immobilizedbiomass of Chlorella sorokiniana characterization studiesrdquoJournal of Hazardous Materials vol 108 no 1-2 pp 85ndash942004

[10] J Wild ldquoLiquid wastes from the metal nishing industryrdquo inSurveys in Industrial Waste Water Treatment D Barnes C FForster and S E Hrudey Eds pp 21ndash62 JohnWiley and SonsNew York NY USA 1987

[11] G H Pino L M S De Mesquita M L Torem and G A SPinto ldquoBiosorption of heavymetals by powder of green coconutshellrdquo Separation Science and Technology vol 41 no 14 pp3141ndash3153 2006

[12] G H Pino L M Souza DeMesquita M L Torem and G A SPinto ldquoBiosorption of cadmiumby green coconut shell powderrdquoMinerals Engineering vol 19 no 5 pp 380ndash387 2006

[13] V K Gupta and A Rastogi ldquoBiosorption of lead(II) fromaqueous solutions by non-living algal biomass Oedogonium spand Nostoc sp a comparative studyrdquo Colloids and Surfaces Bvol 64 no 2 pp 170ndash178 2008

[14] A Kapoor T Viraraghavan and D R Cullimore ldquoRemovalof heavy metals using the fungus Aspergillus nigerrdquo BioresourceTechnology vol 70 no 1 pp 95ndash104 1999

[15] BMattuschka andG Straube ldquoBiosorption ofmetals by awastebiomassrdquo Journal of Chemical Technology and Biotechnologyvol 58 no 1 pp 57ndash63 1993

[16] P Sar S K Kazy R K Asthana and S P Singh ldquoMetal adsorp-tion and desorption by lyophilized Pseudomonas aeruginosardquo


International Biodeterioration and Biodegradation vol 44 no2-3 pp 101ndash110 1999

[17] J M Tobin D G Cooper and R J Neufeld ldquoUptake of metalions by Rhizopus arrhizus biomassrdquo Applied and EnvironmentalMicrobiology vol 47 no 4 pp 821ndash824 1984

[18] H I Al-Taweil M B Osman A A Hamid and W MW Yusoff ldquoOptimizing of Trichoderma viride cultivation insubmerged state fermentationrdquo American Journal of AppliedSciences vol 6 no 7 pp 1284ndash1288 2009

[19] P Anand J Isar S Saran and R K Saxena ldquoBioaccumulationof copper by Trichoderma viriderdquo Bioresource Technology vol97 no 8 pp 1018ndash1025 2006

[20] Metcalf and Eddy Wastewater Engineering Treatment andReuse Tata McGraw-Hill New Delhi India 4th edition 2003

[21] S Lagergren ldquoAbout the theory of so-called adsorption ofsoluble substancesrdquo Kungliga Svenska VetenskapsakademiensHandlingar vol 24 no 4 pp 1ndash39 1898

[22] Y S Ho GMcKay D A JWase and C F Forster ldquoStudy of thesorption of divalent metal ions on to peatrdquo Adsorption Scienceand Technology vol 18 no 7 pp 639ndash650 2000

[23] W J Weber Jr and J C Morriss ldquoKinetics of adsorptionon carbon from solutionrdquo Journal of the Sanitary EngineeringDivision vol 89 no 2 pp 31ndash60 1963

[24] S Wang Y Boyjoo and A Choueib ldquoA comparative studyof dye removal using y ash treated by different methodsrdquoChemosphere vol 60 no 10 pp 1401ndash1407 2005

[25] C K Jain ldquoAdsorption of zinc onto bed sediments of the RiverGanga adsorption models and kineticsrdquo Hydrological SciencesJournal vol 46 pp 419ndash434 2001

[26] Z R Holan and B Volesky ldquoBiosorption of lead and nickel bybiomass ofmarine algaerdquoBiotechnology and Bioengineering vol43 no 11 pp 1001ndash1009 1994

[27] Y Nuhoglu and E Malkoc ldquoermodynamic and kineticstudies for environmentaly friendly Ni(II) biosorption usingwaste pomace of olive oil factoryrdquo Bioresource Technology vol100 no 8 pp 2375ndash2380 2009

[28] M Rao A V Parwate and A G Bhole ldquoRemoval of Cr6+ andNi2+ from aueous solution using bagasse and y ashrdquo WasteManagement vol 22 no 7 pp 821ndash830 2002

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with low cost and complete removal of toxic metals from thewater bodies

In recent years the exploitation of eco-friendly biosorp-tion technology using inactive and dead biomasses to detox-ify metal-contaminated effluents in the aquatic environmentis gaining importance day by day [11 12] Moreover thebiosorbents have high specic metal binding ability incomplex media in contrast to carbonaceous sorbents whichtend to adsorb metal ions in a nonspecic manner eseadvantages make biosorbents an economical alternative tocommercial activated carbons in the removal of heavy metal-polluted water bodies [13]

e application of fungal organisms in the eld ofbiosorption technology has become a part of active researchby the environmental scientists Fungal organisms likeAspergillus niger [14] Streptomyces noursei [15] Pseu-domonas aeruginosa [16] and Rhizopus arrhizus [17] havebeen reported for removal of heavy metals such as PbCd and in particular Ni(II) Among the fungal organismsthe T viride in biosorption process is little exploited [18]e present study in our laboratory is mainly aimed atknowing the application of T viride for sequestration ofNi(II) from contaminated water systems involving kineticand equilibrium e selection of this biosorbent T virideis based on (1) inexpensive (2) easily available (3) no toxiceffects of its own and (4) some information suggests thatmetal-bioaccumulation properties of T viride [19] Hencestudies on the kinetic and equilibrium isotherm modelshave been studied in order to systematically investigatethe application of biomass T viride as biosorbent for theremoval of nickel ions from waterindustrial waste watere optimum conditions for biosorption such as pH initialmetal ion concentration biomass dosage contact time andequilibrium isotherm models in relation to the biosorptionof Ni(II) onto T viride have been investigated In addition tothis the Ni(II) ion desorption studies have been performedover ve sorption-desorption cycles to evaluate the sorbentT viride for reusage

2 Experimental

21 Collection and Preparation of Biomass (Adsorbent) efungal biomass was collected from Microbial Type CultureCollection (MTCC) Chandigarh India e biomass wasprepared in the sabouraud broth (peptone 100 dextrose400 streptomycin 003 and agar 200 gL) by inoculating the01mL spore suspension100mLofwater in the 250mLasksand incubated at room temperature for 5ndash7 days Sampleswere washed several times using deionized water to removeadhesive materials such as extraneous salts and then dried inoven at 60∘C for 48 h and powdered to uniform size using amortar

22 Reagents and Equipments A ame atomic absorptionspectrophotometer (Shimadzu AA-6300 Japan) with nickelhallow cathode lamp was used for determination of Ni(II)before and aer biosorption Absorbance was measured atwavelength of 232 nm and spectral bandwidth was 02 nm

Tra

nsm

itta

nce

(

)

4000 3000 2000 1500 1000 500

33

54

29

24

16

53

14

49 12

44

10

28

63

3


(a) Unloaded

Tra

nsm

itta

nce

(

)

3332

2925

16

42

14

36 1

20

2 57

6

1079

4000 3000 2000 1500 1000 500


(b) Total nickel loaded

F 1 FTIR spectra of T viride biomass before adsorption (a)and aer adsorption of Nickel (b)

Fourier Transform Infrared (FT-IR) spectrometer (ermo-Nicolet FT-IR Nicolet IR-200 USA) was used for IR spectralstudies of dried biomass and Ni(II)-sorbed biomass in therange of 4000ndash400 cmminus1 and Scanning Electron Microscopy(SEM Model Evo15 Carl Zeiss England) has been used tostudy the surface morphology of the biosorbent

3 Results and Discussion

31 Characterization of Biomass e FTIR spectra of freebiomass and nickel sorbed biomass samples were showedin Figure 1 e spectra of free biomass (Figure 1(a)) hasshown a broad and strong peak at 3354 cmminus1 which maybe due to the overlapping of OndashH and NndashH stretchingvibrations e peak at 2924 cmminus1 can be assigned to thendashCH groups of an unloaded biomass sample e peaks at1642 and 1653 cmminus1 may be attributed to asymmetric andsymmetric stretching vibration of C=O groups respectivelye spectrum of nickel sorbed biomass (Figure 1(b)) hasrevealed that the bands that have been observed at 3332 14361202 and 1079 cmminus1 for free biomass are shied to 33541449 1244 and 1028 cmminus1 e signicant changes in thewave numbers of these specic peaks have suggested thatamine hydroxyl C=O and alcoholic CndashO groups of biomasscould be involved in the biosorption of nickel ion onto Tviride

Figure 2 shows the morphology of T viride before andaer biosorption of Ni(II) Before Ni(II) biosorption on Tviride shows adhesive and small particles (Figure 2(a)) It hasbeen shown that the morphology changed to a corn ake-like structure aer Ni(II) biosorption onto T viride biomass


(a)

(b)





100

90

80

70

60

50

40

Ad

sorp

tio

n c

apac

ity

(mg

gminus

1)

0 1 2 3 4 5 6 7

(pH)



50

60

70

80

90

100

110

0 01 02 03 04 05 06 07 08

Rem

ova

l (

)







Ni(II) 00158 09856 0998 00004 0997 0003 2934 09877 094300127 09921 0999 00004 0997 0004 3809 09869 095100134 09968 0999 00004 0999 0003 4559 09713 0934







119905119905119902119902119905119905=111989611989621199021199022119890119890+1119902119902119890119890119905119905 (2)



119902119902119905119905 = 119896119896id11990511990505 + 119888119888 (3)


200

180

160

140

120

100

80

60

40

20

0qt

(mg

gminus

1)

0 2 4 6 8 10 12 14 16

t12

50

100

150

200




SSE = 100557610055761007657100765710076501007650119902119902119905119905119890119890 minus 11990211990211990511990511990511990510076661007666

2

119902119902210076731007673 (4)





119902119902119890119890 =1199021199021198981198981198701198701198711198711198621198621198901198901 + 119870119870119871119871119862119862119890119890

(5)



119902119902119890119890 = 1198961198961198911198911198621198621119899119899119890119890 (6)


1205941205942 = 100557610055761007657100765710076501007650119902119902119890119890 minus 11990211990211989011989011989811989810076661007666

2

11990211990211989011989011989811989810076731007673 (7)



008

007

006

005

004

003

002

001

0

1q

e

1Ce

0 005 01 015 02 025

(a)

2

18

16

14

12

1

08

06

04

02

0

logqe

logCe

0 02 04 0806 1 12 14 16

(b)







293 263 257 0999 1125 4538 1174 0993 512Ni(II) 303 370 315 0999 1728 3566 11047 0999 621

313 476 368 0999 2167 2875 1076 0999 699




4 Conclusion


References

































CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013






(a)

(b)





100

90

80

70

60

50

40

Ad

sorp

tio

n c

apac

ity

(mg

gminus

1)

0 1 2 3 4 5 6 7

(pH)



50

60

70

80

90

100

110

0 01 02 03 04 05 06 07 08

Rem

ova

l (

)







Ni(II) 00158 09856 0998 00004 0997 0003 2934 09877 094300127 09921 0999 00004 0997 0004 3809 09869 095100134 09968 0999 00004 0999 0003 4559 09713 0934







119905119905119902119902119905119905=111989611989621199021199022119890119890+1119902119902119890119890119905119905 (2)



119902119902119905119905 = 119896119896id11990511990505 + 119888119888 (3)


200

180

160

140

120

100

80

60

40

20

0qt

(mg

gminus

1)

0 2 4 6 8 10 12 14 16

t12

50

100

150

200




SSE = 100557610055761007657100765710076501007650119902119902119905119905119890119890 minus 11990211990211990511990511990511990510076661007666

2

119902119902210076731007673 (4)





119902119902119890119890 =1199021199021198981198981198701198701198711198711198621198621198901198901 + 119870119870119871119871119862119862119890119890

(5)



119902119902119890119890 = 1198961198961198911198911198621198621119899119899119890119890 (6)


1205941205942 = 100557610055761007657100765710076501007650119902119902119890119890 minus 11990211990211989011989011989811989810076661007666

2

11990211990211989011989011989811989810076731007673 (7)



008

007

006

005

004

003

002

001

0

1q

e

1Ce

0 005 01 015 02 025

(a)

2

18

16

14

12

1

08

06

04

02

0

logqe

logCe

0 02 04 0806 1 12 14 16

(b)







293 263 257 0999 1125 4538 1174 0993 512Ni(II) 303 370 315 0999 1728 3566 11047 0999 621

313 476 368 0999 2167 2875 1076 0999 699




4 Conclusion


References

































CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013








Ni(II) 00158 09856 0998 00004 0997 0003 2934 09877 094300127 09921 0999 00004 0997 0004 3809 09869 095100134 09968 0999 00004 0999 0003 4559 09713 0934







119905119905119902119902119905119905=111989611989621199021199022119890119890+1119902119902119890119890119905119905 (2)



119902119902119905119905 = 119896119896id11990511990505 + 119888119888 (3)


200

180

160

140

120

100

80

60

40

20

0qt

(mg

gminus

1)

0 2 4 6 8 10 12 14 16

t12

50

100

150

200




SSE = 100557610055761007657100765710076501007650119902119902119905119905119890119890 minus 11990211990211990511990511990511990510076661007666

2

119902119902210076731007673 (4)





119902119902119890119890 =1199021199021198981198981198701198701198711198711198621198621198901198901 + 119870119870119871119871119862119862119890119890

(5)



119902119902119890119890 = 1198961198961198911198911198621198621119899119899119890119890 (6)


1205941205942 = 100557610055761007657100765710076501007650119902119902119890119890 minus 11990211990211989011989011989811989810076661007666

2

11990211990211989011989011989811989810076731007673 (7)



008

007

006

005

004

003

002

001

0

1q

e

1Ce

0 005 01 015 02 025

(a)

2

18

16

14

12

1

08

06

04

02

0

logqe

logCe

0 02 04 0806 1 12 14 16

(b)







293 263 257 0999 1125 4538 1174 0993 512Ni(II) 303 370 315 0999 1728 3566 11047 0999 621

313 476 368 0999 2167 2875 1076 0999 699




4 Conclusion


References

































CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013







119902119902119890119890 =1199021199021198981198981198701198701198711198711198621198621198901198901 + 119870119870119871119871119862119862119890119890

(5)



119902119902119890119890 = 1198961198961198911198911198621198621119899119899119890119890 (6)


1205941205942 = 100557610055761007657100765710076501007650119902119902119890119890 minus 11990211990211989011989011989811989810076661007666

2

11990211990211989011989011989811989810076731007673 (7)



008

007

006

005

004

003

002

001

0

1q

e

1Ce

0 005 01 015 02 025

(a)

2

18

16

14

12

1

08

06

04

02

0

logqe

logCe

0 02 04 0806 1 12 14 16

(b)







293 263 257 0999 1125 4538 1174 0993 512Ni(II) 303 370 315 0999 1728 3566 11047 0999 621

313 476 368 0999 2167 2875 1076 0999 699




4 Conclusion


References

































CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013








293 263 257 0999 1125 4538 1174 0993 512Ni(II) 303 370 315 0999 1728 3566 11047 0999 621

313 476 368 0999 2167 2875 1076 0999 699




4 Conclusion


References

































CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013





















CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013







CatalystsJournal of














Journal of

SPECTROSCOPY






Advances in

Physical Chemistry

ISRN Chromatography







Journal of

Chemistry







Journal of

Volume 2013





Documents

Effective Biosorption of Nickel(II) From Aqueous Solutions Using Trichoderma Viride